Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations
|
|
- Louisa Goodwin
- 6 years ago
- Views:
Transcription
1 Chemistry, The Central Science, 10th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 3 : Calculations with Chemical Formulas and Equations John D. Bookstaver St. Charles Community College St. Peters, MO 2006, Prentice-Hall
2 Law of Conservation of Mass We may lay it down as an incontestable axiom that, in all the operations of art and nature, nothing is created; an equal amount of matter exists both before and after the experiment. Upon this principle, the whole art of performing chemical experiments depends. --Antoine Lavoisier, 1789
3 Chemical Equations Concise representations of chemical reactions
4 Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g)
5 Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Reactants appear on the left side of the equation.
6 Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Products appear on the right side of the equation.
7 Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) The states of the reactants and products are written in parentheses to the right of each compound.
8 Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Coefficients are inserted to balance the equation.
9 Subscripts and Coefficients Give Different Information Subscripts tell the number of atoms of each element in a molecule
10 Subscripts and Coefficients Give Different Information Subscripts tell the number of atoms of each element in a molecule Coefficients tell the number of molecules
11 Reaction Types
12 Combination Reactions Two or more substances react to form one product Examples: N 2 (g) + 3 H 2 (g) 2 NH 3 (g) C 3 H 6 (g) + Br 2 (l) C 3 H 6 Br 2 (l) 2 Mg (s) + O 2 (g) 2 MgO (s)
13 2 Mg (s) + O 2 (g) 2 MgO (s)
14 Decomposition Reactions One substance breaks down into two or more substances Examples: CaCO 3 (s) CaO (s) + CO 2 (g) 2 KClO 3 (s) 2 KCl (s) + O 2 (g) 2 NaN 3 (s) 2 Na (s) + 3 N 2 (g)
15 Combustion Reactions Examples: Rapid reactions that produce a flame Most often involve hydrocarbons reacting with oxygen in the air CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) C 3 H 8 (g) + 5 O 2 (g) 3 CO 2 (g) + 4 H 2 O (g)
16 Formula Weights
17 Formula Weight (FW) Sum of the atomic weights for the atoms in a chemical formula So, the formula weight of calcium chloride, CaCl 2, would be Ca: 1(40.1 amu) + Cl: 2(35.5 amu) amu These are generally reported for ionic compounds
18 Molecular Weight (MW) Sum of the atomic weights of the atoms in a molecule For the molecule ethane, C 2 H 6, the molecular weight would be C: 2(12.0 amu) + H: 6(1.0 amu) 30.0 amu
19 Percent Composition One can find the percentage of the mass of a compound that comes from each of the elements in the compound by using this equation: % element = (number of atoms)(atomic weight) (FW of the compound) x 100
20 Percent Composition So the percentage of carbon in ethane is %C = (2)(12.0 amu) (30.0 amu) 24.0 amu = x amu = 80.0%
21 Moles
22 Avogadro s Number 6.02 x mole of 12 C has a mass of 12 g
23 Molar Mass By definition, these are the mass of 1 mol of a substance (i.e., g/mol) The molar mass of an element is the mass number for the element that we find on the periodic table The formula weight (in amu s) will be the same number as the molar mass (in g/mol)
24 Using Moles Moles provide a bridge from the molecular scale to the real-world scale
25 Mole Relationships One mole of atoms, ions, or molecules contains Avogadro s number of those particles One mole of molecules or formula units contains Avogadro s number times the number of atoms or ions of each element in the compound
26 Finding Empirical Formulas
27 Calculating Empirical Formulas One can calculate the empirical formula from the percent composition
28 Calculating Empirical Formulas The compound para-aminobenzoic acid (you may have seen it listed as PABA on your bottle of sunscreen) is composed of carbon (61.31%), hydrogen (5.14%), nitrogen (10.21%), and oxygen (23.33%). Find the empirical formula of PABA.
29 Calculating Empirical Formulas Assuming g of para-aminobenzoic acid, C: g x 1 mol = mol C g H: 5.14 g x 1 mol 1.01 g = 5.09 mol H N: 1 mol g x g = mol N O: 1 mol g x g = mol O
30 Calculating Empirical Formulas Calculate the mole ratio by dividing by the smallest number of moles: mol C: = mol 5.09 mol H: = mol mol N: = mol mol O: = mol
31 Calculating Empirical Formulas These are the subscripts for the empirical formula: C 7 H 7 NO 2
32 Combustion Analysis Compounds containing C, H and O are routinely analyzed through combustion in a chamber like this C is determined from the mass of CO 2 produced H is determined from the mass of H 2 O produced O is determined by difference after the C and H have been determined
33 Elemental Analyses Compounds containing other elements are analyzed using methods analogous to those used for C, H and O
34 Stoichiometric Calculations The coefficients in the balanced equation give the ratio of moles of reactants and products
35 Stoichiometric Calculations From the mass of Substance A you can use the ratio of the coefficients of A and B to calculate the mass of Substance B formed (if it s a product) or used (if it s a reactant)
36 Stoichiometric Calculations C 6 H 12 O O 2 6 CO H 2 O Starting with 1.00 g of C 6 H 12 O 6 we calculate the moles of C 6 H 12 O 6 use the coefficients to find the moles of H 2 O and then turn the moles of water to grams
37 Limiting Reactants
38 How Many Cookies Can I Make? You can make cookies until you run out of one of the ingredients Once this family runs out of sugar, they will stop making cookies (at least any cookies you would want to eat)
39 How Many Cookies Can I Make? In this example the sugar would be the limiting reactant, because it will limit the amount of cookies you can make
40 Limiting Reactants The limiting reactant is the reactant present in the smallest stoichiometric amount
41 Limiting Reactants The limiting reactant is the reactant present in the smallest stoichiometric amount In other words, it s the reactant you ll run out of first (in this case, the H 2 )
42 Limiting Reactants In the example below, the O 2 would be the excess reagent
43 Theoretical Yield The theoretical yield is the amount of product that can be made In other words it s the amount of product possible as calculated through the stoichiometry problem This is different from the actual yield, the amount one actually produces and measures
44 Percent Yield A comparison of the amount actually obtained to the amount it was possible to make Actual Yield Percent Yield = x 100 Theoretical Yield
Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations
Chemistry, The Central Science, 10th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 3 : Calculations with Chemical Formulas and Equations John D. Bookstaver St. Charles Community
More informationChapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 3 : Calculations with Chemical Formulas and Equations John D. Bookstaver St. Charles Community
More informationChapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations. Lecture Presentation
Lecture Presentation Chapter 3 : Calculations with Chemical Formulas and Equations John D. Bookstaver St. Charles Community College Cottleville, MO Law of Conservation of Mass We may lay it down as an
More informationChapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations
Chapter 3 : Calculations with Chemical Formulas and Equations AP Chemistry 2014-15 North Nova Education Centre Mr. Gauthier Law of Conservation of Mass We may lay it down as an incontestable axiom that,
More informationChemical Equations. Law of Conservation of Mass. Anatomy of a Chemical Equation CH4(g) + 2O2(g) Chapter 3
Chemical Equations Chemical equations are concise representations of chemical reactions. Chapter 3 : Calculations with Chemical Formulas and Equations Law of Conservation of Mass Anatomy of a Chemical
More informationChapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations. Stoichiometry
Chapter 3 : Calculations with Chemical Formulas and Equations Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2
More informationChapter 3: Stoichiometry
Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and
More informationChapter 3 Chemical Reactions and Reaction Stoichiometry
Chapter 3 Chemical Reactions and Reaction Stoichiometry 2015 Pearson Education, Inc. Chemical Reactions and Reaction Stoichiometry 3.1 Chemical Equations 3.2 Simple Patterns of Chemical Reactivity 3.3
More informationPowerPoint to accompany. Chapter 2. Stoichiometry: Calculations with Chemical Formulae and Equations. Dr V Paideya
PowerPoint to accompany Chapter 2 Stoichiometry: Calculations with Chemical Formulae and Equations Dr V Paideya Chemical Equations CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Figure 2.4 Chemical Equations
More informationChapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations. Lecture Presentation
Lecture Presentation Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations John D. Bookstaver St. Charles Community College Cottleville, MO A. 1 Mg, 2 O, and 2 H B. 2 Mg, 2 O, and
More informationChapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations
Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations Matter Matter is anything that has mass and takes up space 2 Composition of Matter Atom number of protons = atomic number (Z)
More informationChapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations
Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations Lecture Outline 3.1 Chemical Equations The quantitative nature of chemical formulas and reactions is called stoichiometry. Lavoisier
More informationCartoon courtesy of NearingZero.net. Stoichiometry
Cartoon courtesy of NearingZero.net Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Reactants appear on the left side of the equation. Anatomy of a Chemical Equation CH 4 (g)
More information3 Stoichiometry: Calculations with Chemical Formulas and Equations
3 Stoichiometry: Calculations with Chemical Formulas and Equations 3.1 Chemical Equations Balance chemical equations. 3. Simple Patterns of Reactivity Predict products of a chemical reaction in a combination
More informationAP Chemistry Chapter 3. Stoichiometry
AP Chemistry Chapter 3 Stoichiometry Stoichiometry Is the study of the quantities of substances consumed and produced in chemical reactions Derived from the Greek words stoicheion meaning element and metron
More informationStoichiometry Dr. M. E. Bridge
Preliminary Chemistry Course Stoichiometry Dr. M. E. Bridge What is stoichiometry? The meaning of the word: The word stoichiometry comes from two Greek words: stoichon(meaning element ) and metron(meaning
More informationChapter 3. Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions In this chapter, Chemical structure and formulas in studying the mass relationships of atoms and molecules. To explain the composition of compounds and
More informationStoichiometry CHAPTER 12
CHAPTER 12 Stoichiometry 12.1 Using Everyday Equations Stoichiometry is the calculation of quantities in chemical equations. * The balanced equation gives the ratios for the reactants and products. 3 eggs
More informationMass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
More informationStoichiometry CHAPTER 12
CHAPTER 12 Stoichiometry 12.1 Using Everyday Equations Stoichiometry is the calculation of quantities in chemical equations. Jan 16 7:57 AM May 24 10:03 AM * The balanced equation gives the ratios for
More informationGeneral Chemistry. Chapter 3. Mass Relationships in Chemical Reactions CHEM 101 (3+1+0) Dr. Mohamed El-Newehy 10/12/2017
General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 3 Mass Relationships in Chemical Reactions 1 In this chapter, Chemical structure and formulas in studying
More informationCHAPTER 12. Chemists use balanced to calculate how much reactant is needed or product is formed in a reaction. + 3H 2NH. Hon Chem 12.
CHAPTER 12 Stoichiometry is the calculation of quantities using different substances in chemical equations. Based on the Law of Conservation of Mass. Mg(s) + How many moles of H Chemists use balanced to
More informationMass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
More informationMass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
More informationMatter, Measurement, & Stoichiometry
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Unit 3 (Chp 1,2,3): Matter, Measurement, & Stoichiometry John D. Bookstaver St. Charles Community
More informationStoichiometry. Please take out your notebooks
Stoichiometry Please take out your notebooks Stoichiometry stochio = Greek for element metry = measurement Stoichiometry is about measuring the amounts of elements and compounds involved in a reaction.
More informationMass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
More informationMoles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Micro World atoms & molecules Macro World grams Atomic mass is the mass of an atom in
More informationSolutions to the Extra Problems for Chapter 8
Solutions to the Extra Problems for Chapter 8. The answer is 83.4%. To figure out percent yield, you first have to determine what stoichiometry says should be made: Mass of MgCl 4.3 amu + 35.45 amu 95.
More informationChapter 3. Stoichiometry:
Chapter 3. Stoichiometry: Watch Bozeman Videos & other videos on my website for additional help: Big Idea 1: Chemical Analysis Conservation of Atoms Balancing Equations Symbolic Representation Mole Big
More informationCHEMICAL ARITHMATICS MODULE - 1. Objectives. Chemical Arithmatics. Atoms, Molecules and Chemical Arithmatics. Notes
2 MODULE - 1 CHEMICAL ARITHMATICS W e know that atoms of different elements combine in simple whole-number ratios to form molecules. For example, hydrogen and oxygen atoms combine in the mass ratio of
More informationChemistry 101 Chapter 8 Chemical Composition
Chemistry 101 Chapter 8 Chemical Composition Atomic mass unit (amu): a unit of the scale relative masses of atoms (1 amu = 1.66 10-24 g). Atomic weight (Atomic mass): the atomic weight of an element given
More informationStoichiometry. Chapter 3
Stoichiometry Chapter 3 Chemical Stoichiometry Stoichiometry: The study of quantities of materials consumed and produced in chemical reactions. In macroworld, we can count objects by weighing assuming
More informationChemical Equations and Chemical Reactions
Chemical Equations Chemical Equations and Chemical Reactions Chemical equations are concise representations of chemical reactions. Chemical Equations Symbols Used in Chemical Equations The formulas of
More informationMatter, Measurement, & Stoichiometry
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Unit 3 (Chp 1,2,3): Matter, Measurement, & Stoichiometry John D. Bookstaver St. Charles Community
More informationThe Mole. Relative Atomic Mass Ar
STOICHIOMETRY The Mole Relative Atomic Mass Ar Relative Molecular Mass Mr Defined as mass of one atom of the element when compared with 1/12 of an atom of carbon-12 Some Ar values are not whole numbers
More informationCHAPTER 11. The Mole. Mole. One mole of = 6.02 x 10 = 6.02 x 10 CaCl = 6.02 x x 10. Representative Particle. molecules, or formula units
CHAPTER 11 The Mole 11.1 The Mole: Measurement of Matter Matter is measured in one of three ways: (How many?) Mole SI unit that measures the amount of a substance 6.02 x 10 particles of that substance.
More informationReactants and products. Indications of state. Mass balance: coefficients vs. subscripts
1 of 9 I. Chemical equations Chemical equations - shorthand representations of chemical reactions The reaction of aqueous silver (I) nitrate and aqueous ammonium chloride results in the formation of solid
More information9/14/ Chemistry Second Edition Julia Burdge. Stoichiometry: Ratios of Combination. Molecular and Formula Masses
9/14/1 Chemistry Second Edition Julia Burdge Stoichiometry: Ratios of Combination Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Stoichiometry: Ratios
More informationChapter 1 IB Chemistry Warm Ups Stoichiometry. Mrs. Hilliard
Chapter 1 IB Chemistry Warm Ups Stoichiometry Mrs. Hilliard Vocabulary 1. Atomic theory 2. Kelvin 3. Mole 4. Relative abundance 5. Molar Mass 6. Empirical formula 7. Molecular formula 8. Stoichiometry
More informationDo Now. Agenda Welcome back! The beginning of ALL THE MATH! Homework PBJ procedure Pages 1-3 of HW packet
Do Now Agenda Welcome back! The beginning of ALL THE MATH! Homework PBJ procedure Pages 1-3 of HW packet All the math Molar Mass the mass of one mole of any substance, reported in grams (gram atomic mass)
More informationUNIT 1 Chemical Reactions Part II Workbook. Name:
UNIT 1 Chemical Reactions Part II Workbook Name: 1 Molar Volume 1. How many moles of a gas will occupy 2.50 L at STP? 2. Calculate the volume that 0.881 mol of gas at STP will occupy. 3. Determine the
More informationChemical Reactions, Chemical Equations, and Stoichiometry. Brown, LeMay Ch 3 AP Chemistry
Chemical Reactions, Chemical Equations, and Stoichiometry Brown, LeMay Ch 3 AP Chemistry 1 3.: Types of reactions http://web.fuhsd.org/kavita_gupta/july.html 3.3: Atomic, Molecular & Formula Weights Atomic
More informationStoichiometry World of Chemistry: Chapter 9
Stoichiometry World of Chemistry: Chapter 9 Chocolate Chip Cookies!! 1 cup butter 1/2 cup white sugar 1 cup packed brown sugar 1 teaspoon vanilla extract 2 eggs 2 1/2 cups all-purpose flour 1 teaspoon
More informationCh. 3 The Mole: Relating the Microscopic World of Atoms to Laboratory Measurements. Brady & Senese, 5th Ed.
Ch. 3 The Mole: Relating the Microscopic World of Atoms to Laboratory Measurements Brady & Senese, 5th Ed. Index 3.1 The mole conveniently links mass to number of atoms or molecules 3.2 Chemical formulas
More information2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with
Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12
More informationStoichiometry. Introduction. Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Avogadros Number: (number of Molecules)
Stoichiometry Introduction Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Or Avogadros Number: (number of Molecules) Or Moles (amount of a substance containing avogadros number
More informationFinding Formulas. using mass information about a compound to find its formula
Finding Formulas using mass information about a compound to find its formula Molecular Formula Molecular formula is the actual formula of compounds which form molecules. For example, the molecular formula
More information2.9 The Mole and Chemical Equations:
2.9 The Mole and Chemical Equations: Stoichiometry Whether you are making omelettes in a kitchen or soap in a factory, you need to know the quantities of ingredients required to produce a certain quantity
More informationChapter 3. Chemical Equations & Reaction Stoichiometry. Symbolic representation of a chemical reaction
Chapter 3 Chemical Equations & Reaction Stoichiometry I) Chemical Equations Symbolic representation of a chemical reaction potassium + water v potassium hydroxide + hydrogen 2 K(s) + 2 H 2 O(R)! 2 KOH(aq)
More informationCHEMICAL FORMULA COEFFICIENTS AND SUBSCRIPTS 3O 2 2O 3. ! Formula that gives the TOTAL number of elements in a molecule or formula unit.
CHEMICAL FORMULA! Formula that gives the TOTAL number of elements in a molecule or formula unit. No Score from Exam 1? Go to 210 Whitmore and speak with Mike Joyce to get it straightened out. Which Skill
More informationHonors Chemistry Unit 6 Moles and Stoichiometry Notes. Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number?
Honors Chemistry Unit 6 Moles and Stoichiometry Notes Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number? 3. What does it mean? 4. How is a mole like a dozen doughnuts? Formula
More informationQuantity Relationships in Chemical Reactions
Chapter 10 Relationships in Chemical Reactions Section 10.1 Conversion Factors from a Chemical Equation Goal 1 The coefficients in a chemical equation give us the conversion factors to get from the number
More informationCh 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances.
Ch 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances. Moles the SI base unit that describes the amount of particles in a substance. Mole is abbreviated
More informationQ: How long would it take to spend a mole of $1 coins if they were being spent at a rate of 1 billion per second? A:
: The Mole- 6.02 x 10 23 ODE TO A MOLE I find that my heart beat goes out of control Just thinking how useful to man is the mole! So perfectly compact. What could be neater? Only occupying twenty-two and
More informationStoichiometry Ratios of Combination
Chapter 3 Stoichiometry Ratios of Combination Dr. A. Al-Saadi 1 Preview Concepts of atomic mass, molecular mass, mole, molar mass, and percent compositions. Balancing chemical equations. Stoichiometric
More informationUNIT 3 IB MATERIAL BONDING, MOLES & STOICHIOMETRY
UNIT 3 IB MATERIAL Name: BONDING, MOLES & STOICHIOMETRY ESSENTIALS: Know, Understand, and Be Able To Apply the mole concept to substances. Determine the number of particles and the amount of substance
More informationThe coefficients of a balanced chemical equation tell us how many of each species are involved in the reaction.
Stoichiometry Chemical Equations Reactants are written on the left side of the arrow and products are written on the right side of the arrow. The Law of Conservation of Mass tells us that the number of
More informationName Date Class STOICHIOMETRY. SECTION 12.1 THE ARITHMETIC OF EQUATIONS (pages )
Name Date Class 1 STOICHIOMETRY SECTION 1.1 THE ARITHMETIC OF EQUATIONS (pages 353 358) This section explains how to calculate the amount of reactants required or product formed in a nonchemical process.
More informationLIMITING REAGENT. Taking Stoichiometric conversions one step further
LIMITING REAGENT Taking Stoichiometric conversions one step further Limiting Reagent The reactant that limits the amount of product that can be formed. The reaction will stop when all of the limiting reactant
More informationAP Chemistry: Chapter 3 Notes Outline
AP Chemistry: Chapter 3 Notes Outline Objectives: Balance chemical equations Use dimensional analysis to solve stoichiometric problems Use dimensional analysis to do limiting reactant problems Use dimensional
More informationChapter 3. Stoichiometry
Chapter 3 Stoichiometry Chapter 3 Chemical Stoichiometry Stoichiometry The study of quantities of materials consumed and produced in chemical reactions. Since atoms are so small, we must use the average
More informationName: Class: Date: SHORT ANSWER Answer the following questions in the space provided.
CHAPTER 9 REVIEW Stoichiometry SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. The coefficients in a chemical equation represent the (a) masses in grams of all reactants
More informationA TAKAMUL INTERNATIONAL SCHOOL CH.10 THE MOLE PREPARED BY MR. FAHAD AL-JARAH
A TAKAMUL INTERNATIONAL SCHOOL CH.10 THE MOLE PREPARED BY MR. FAHAD AL-JARAH Chapter Outline Section 10.1 Measuring Matter Key Concepts The mole is a unit used to count particles of matter indirectly.
More informationUNIT 6 STOICHIOMETRY 1
UNIT 6 STOICHIOMETRY 1 There are three ways to measure matter count (number of particles representative particles) mass (grams) volume (Liters) Mole unit for amt of matter relating these quantities 2 Representative
More information1.3: Empirical and Molecular Formulas. Ms. Kiely Coral Gables Senior High IB Chemistry SL
1.3: Empirical and Molecular Formulas Ms. Kiely Coral Gables Senior High IB Chemistry SL Practice How heavy are 1.20 x 10²⁵ atoms of potassium? ANSWER How many grams in 1.20 x 10²⁵ atoms of potassium?
More informationChemistry I Notes Unit 7: Stoichiometry Notes
Chemistry I Notes Unit 7: Stoichiometry Notes Stoichiometry Relating Mass to Numbers of Atoms The Mole The mole is the SI unit for amount of substance. A mole (abbreviated mol) is the amount of a substance
More informationStoichiometry (Chapter 3)
Stoichiometry (Chapter 3) Antoine Lavoisier eperimental observations lead to the development of the Law of Conservation of Mass (a.k.a. Law of Conservation of Matter). The updated version of the law of
More informationNotes: Unit 7 Moles & Stoichiometry
Regents Chemistry: Notes: Unit 7 Moles & Stoichiometry 1 KEY IDEAS A compound is a substance composed of two or more different elements that are chemically combined in a fixed proportion. A chemical compound
More informationChapter 3 Stoichiometry. Ratios of combination
Chapter 3 Stoichiometry Ratios of combination Topics Molecular and formula masses Percent composition of compounds Chemical equations Mole and molar mass Combustion analysis (Determining the formula of
More informationChapter 9. Stoichiometry. Mr. Mole. NB page 189
Chapter 9 Stoichiometry Mr. Mole NB page 189 review Let s make some Cookies! When baking cookies, a recipe is usually used, telling the exact amount of each ingredient. If you need more, you can double
More informationChemical Calculations: The Mole concept and Chemical Formula. Law of Definite Proportions (John Dalton) Chapter 9
Chapter 9 Chemical Calculations: The Mole concept and Chemical Formula This material is not included in Midterm 1 1 Law of Definite Proportions (John Dalton) Chapter 9 A given compound always contains
More informationLecture 11 - Stoichiometry. Lecture 11 - Introduction. Lecture 11 - The Mole. Lecture 11 - The Mole. Lecture 11 - The Mole
Chem 103, Section F0F Unit IV - Stoichiometry of Formulas and Equations Lecture 11 The concept of a mole, which is a very large group of atoms or molecules Determining the formulas for a compound Stoichiometry
More informationMass Relationships in Chemical Reactions
Reading Assignments: Chapter 3 in R. Chang, Chemistry, 8th Ed., McGraw-Hill, 2005 Mass Relationships in Chemical Reactions Or Related topics in other textbooks. Consultation outside lecture room: Office
More informationProportional Relationships
Stoichiometry Video Proportional Relationships 2 1/4 c. flour 1 tsp. baking soda 1 tsp. salt 1 c. butter 3/4 c. sugar 3/4 c. brown sugar 1 tsp vanilla extract 2 eggs 2 c. chocolate chips Makes 5 dozen
More informationHow many molecules are in 0.25 moles of CH 4?
Mass Moles- Particle Particles can be atoms, molecules, ions, etc. In one mole of particles, there are 6.02x10 23 particles These particles are so small and we need so many of them to be on a human scale,
More informationChapter 3 Calculations with Chemical Formulas and Equations
Chapter 3 Calculations with Chemical Formulas and Equations Contents and Concepts Mass and Moles of Substances Here we will establish a critical relationship between the mass of a chemical substance and
More informationChapter 3: Chemical Reactions and the Earth s Composition
Chapter 3: Chemical Reactions and the Earth s Composition Problems: 3.1-3.3, 3.5, 3.11-3.86, 3.95-3.115, 3.119-3.120, 3.122, 3.125-3.128, 3.132, 3.134, 3.136-3.138-3.141 3.2 The Mole Stoichiometry (STOY-key-OM-e-tree):
More informationNotes: Unit 7 Moles & Stoichiometry
Regents Chemistry: Notes: Unit 7 Moles & Stoichiometry 1 KEY IDEAS In all chemical reactions there is a conservation of mass, energy, and charge. (3.3a) A balanced chemical equation represents conservation
More informationChemistry Section Review 7.3
Chemistry Section Review 7.3 Multiple Choice Identify the choice that best completes the statement or answers the question. Put the LETTER of the correct answer in the blank. 1. The molar mass of an element
More informationAtoms, Ions and Molecules Calculations
Atoms, Ions and Molecules Calculations 1. How do you calculate the atomic mass of an element? Atomic Mass = (% abundance of isotope 1)(mass of isotope 1) + (% abundance of isotope2)(mass of isotope 2)
More informationProblem Set III Stoichiometry - Solutions
Chem 121 Problem set III Solutions - 1 Problem Set III Stoichiometry - Solutions 1. 2. 3. molecular mass of ethane = 2(12.011) + 6(1.008) = 30.07 g 4. molecular mass of aniline = 6(12.011) + 7(1.008) +
More informationAtoms, Molecules, and the Mole
The Mole Now that we know how to write and name chemical compounds, we need to understand how chemists use these formulas quantitatively. As chemists, we need to know how many atoms or molecules are reacting
More informationCounting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles
Unit 8: Quantification of Chemical Reactions Chapter 10: The mole Chapter 12: Stoichiometry Counting by mass: The Mole Chemists can t count individual atoms Use moles to determine amounts instead mole
More informationWhat is a Representative Particle
Chapter 7 Moles What is a Representative Particle The smallest unit into which a substance can be broken down without changing the composition of the substance. Atoms, molecules, and formula units What
More informationCalculations with Chemical Formulas and Equations
Calculations with Chemical Formulas and Equations Mass and Moles of a Substance Chemistry requires a method for determining the numbers of molecules in a given mass of a substance. This allows the chemist
More informationChemical Equations. Chemical Equations
Page III-4a-1 / Chapter Four Part I Lecture Notes Chemical Reactions Chapter 4 Part 1 Chemistry as Cooking! - the Chemical Reaction "Recipe" and technique leads to successful creations Must know amounts
More informationLecture 0503 Calorimetry and Hess s Law
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Lecture 0503 Calorimetry and Hess s Law John D. Bookstaver St. Charles Community College Cottleville,
More informationMolar Mass. The total of the atomic masses of all the atoms in a molecule:
Molar Mass The total of the atomic masses of all the atoms in a molecule: Ex: H 2 O H (1.0079) x 2 atoms = 2.0158 grams O (15.999) x 1 atom = 15.999 grams 18.0148 grams (18.0 grams) Ex: Cu(NO 3 ) 2 Cu
More informationClass XI Chapter 1 Some Basic Concepts of Chemistry Chemistry
Question 1.1: Calculate the molecular mass of the following: (i) H 2 O (ii) CO 2 (iii) CH 4 (i) H 2 O: The molecular mass of water, H 2 O = (2 Atomic mass of hydrogen) + (1 Atomic mass of oxygen) = [2(1.0084)
More informationChapter 10 Chemical Quantities
Chapter 10 Chemical Quantities 10.1 The Mole: A Measurement of Matter OBJECTIVES: Describe methods of measuring the amount of something. Define Avogadro s number as it relates to a mole of a substance.
More informationWorksheet 1: REPRESENTATIVE PARTICLES
Worksheet 1: REPRESENTATIVE PARTICLES Directions: For each substance below, state the representative particle. If the RP is a molecule, state the number of atoms that make up the molecule. If the RP is
More informationStoichiometry Dry Lab
Stoichiometry Dry Lab Name: Mole-Mass Conversions The molar mass of a substance is the conversion factor that allows us to convert between the mass of a substance (in grams) and the number of moles of
More informationMass Relationship in Chemical Reaction
CHEMISTRY - DMCU 1233 Fakulti Kejuruteraan Mekanikal, UTeM Lecturer: IMRAN SYAKIR BIN MOHAMAD MOHD HAIZAL BIN MOHD HUSIN NONA MERRY MERPATI MITAN Mass Relationship in Chemical Reaction Chapter 3 1 Atomic
More informationSTOICHIOMETRY. Measurements in Chemical Reactions
STOICHIOMETRY Measurements in Chemical Reactions STOICHIOMETRY Stoichiometry is the analysis of the quantities of substances in a chemical reaction. Stoichiometric calculations depend on the MOLE-MOLE
More informationStoichiometry Dry Lab
Stoichiometry Dry Lab Name: Mole-Mass Conversions The molar mass of a substance is the conversion factor that allows us to convert between the mass of a substance (in grams) and the number of moles of
More informationUnit 10: Stoichiometry. Stoichiometry= the process of using a to determine the relative amounts of reactants and products involved in a reaction.
Unit 10: Stoichiometry Stoichiometry= the process of using a to determine the relative amounts of reactants and products involved in a reaction. Info given by a chemical equation: Chemical changes involve
More information**continued on next page**
Chapter 9 Stoichiometry Section 9.1 Introduction to Stoichiometry Standard.e.: Students know how to calculate the masses of reactant and products in a chemical reaction from the mass of one of the reactants
More informationChapter 3: Molecules, Compounds and Chemical Equations: (continue and finish chapter 3: 8-11)
C h e m i s t r y 1 A : C h a p t e r 3 P a r t B P a g e 1 Chapter 3: Molecules, Compounds and Chemical Equations: (continue and finish chapter 3: 8-11) Homework: Read Chapters 3. Work out sample/practice
More informationChapter 3 Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions Semester 1/2012 3.1 Atomic Mass 3.2 Avogadro s Number and the Molar Mass of an element 3.3 Molecular Mass 3.5 Percent Composition of Compounds 3.6 Experimental
More information